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Chapter 9: Problem 49

Complete and balance the following equations. If no reaction occurs, so state. (a) \(\operatorname{Rb}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(1) \longrightarrow\) (b) \(\mathrm{I}_{2}(\mathrm{s})+\mathrm{Na}^{+}(\mathrm{aq})+\mathrm{Br}^{-}(\mathrm{aq}) \longrightarrow\) (c) \(\operatorname{SrO}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(1) \longrightarrow\) (d) \(\mathrm{SO}_{3}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(1) \longrightarrow\)

Short Answer

Expert verified
The balanced equations are: (a) \(2 \operatorname{Rb}(\mathrm{s})+2\mathrm{H}_{2} \mathrm{O}(1) \longrightarrow 2\operatorname{RbOH}(\mathrm{aq}) + \mathrm{H}_{2}(\mathrm{g})\), (b) No reaction, (c) \(\operatorname{SrO}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(1) \longrightarrow \operatorname{Sr(OH)}_2(\mathrm{aq})\), (d) \(\mathrm{SO}_{3}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(1) \longrightarrow \mathrm{H}_{2}\mathrm{SO}_{4}(\mathrm{g})\).

Step by step solution

01

Equation (a) Balancing

First, let's analyze equation (a) - \(\operatorname{Rb}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(1) \longrightarrow\). Rb is Rubidium, a metal that reacts with water (H2O) vigorously producing Hydrogen gas (H2) and Rubidium hydroxide (RbOH). The balanced equation for this reaction is \(2 \operatorname{Rb}(\mathrm{s})+2\mathrm{H}_{2} \mathrm{O}(1) \longrightarrow 2\operatorname{RbOH}(\mathrm{aq}) + \mathrm{H}_{2}(\mathrm{g})\).
02

Equation (b) Assessment

For equation (b) - \(\mathrm{I}_{2}(\mathrm{s})+\mathrm{Na}^{+}(\mathrm{aq})+\mathrm{Br}^{-}(\mathrm{aq}) \longrightarrow\), iodine (I2) is a halogen, but since it's less reactive than bromine (Br), a single-displacement reaction won't occur. Therefore, no reaction happens here.
03

Equation (c) Balancing

Looking at equation (c) - \(\operatorname{SrO}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(1) \longrightarrow\), Strontium oxide (SrO) is a metal oxide which reacts with water to form a base. In this case it forms Sr(OH)2. The balanced chemical equation is \(\operatorname{SrO}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(1) \longrightarrow \operatorname{Sr(OH)}_2(\mathrm{aq})\).
04

Equation (d) Balancing

Finally, let's look at equation (d) - \(\mathrm{SO}_{3}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(1) \longrightarrow\). Here, Sulphur trioxide (SO3) reacts with water (H2O) to form H2SO4 (sulphuric acid), so the reaction is: \(\mathrm{SO}_{3}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(1) \longrightarrow \mathrm{H}_{2}\mathrm{SO}_{4}(\mathrm{g})\).

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Most popular questions from this chapter

Which of the following ions are likely to be found in chemical compounds: \(\mathrm{Na}^{2+}, \mathrm{Li}^{+}, \mathrm{Al}^{4+}, \mathrm{F}^{2-},\) or \(\mathrm{Te}^{2-} ?\) Explain briefly.

Describe how the ionization energies of the ions \(\mathrm{He}^{-}, \mathrm{Li}^{-}, \mathrm{Be}^{-}, \mathrm{B}^{-}, \mathrm{C}^{-}, \mathrm{N}^{-}, \mathrm{O}^{-},\) and \(\mathrm{F}^{-}\) vary with atomic number.

All the isoelectronic species illustrated in the text had the electron configurations of noble gases. Can two ions be isoelectronic without having noble-gas electron configurations? Explain.

Indicate the smallest and the largest species (atom or ion) in the following group: Al atom, F atom, As atom, \(\mathrm{Cs}^{+}\) ion, \(\mathrm{I}^{-}\) ion, \(\mathrm{N}\) atom.

Briefly describe each of the following ideas or phenomena: (a) the periodic law; (b) ionization energy; (c) electron affinity; (d) paramagnetism.
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